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Ch.4 - Reactions in Aqueous Solution
Brown - Chemistry: The Central Science 15th Edition
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Tutti i libri di testoBrown 15th EditionCh.4 - Reactions in Aqueous SolutionProblema 39
Capitolo 4, Problema 39

Complete and balance the following molecular equations, and then write the net ionic equation for each:
(a) HBr(aq) + Ca(OH)2(aq) →
(b) Cu(OH)2(s) + HClO4(aq) →
(c) Al(OH)3(s) + HNO3(aq) →

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Identify the reactants and products in the given molecular equation: Cu(OH)_2(s) + HClO_4(aq).
Write the balanced molecular equation by ensuring the number of atoms of each element is the same on both sides of the equation.
Dissociate all strong electrolytes into their ions. In this case, HClO_4 is a strong acid and will dissociate into H^+ and ClO_4^- ions.
Identify the solid, liquid, or gas products that do not dissociate into ions. Cu(OH)_2 is a solid and does not dissociate.
Write the net ionic equation by removing the spectator ions (ions that appear on both sides of the equation) from the complete ionic equation.

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Balancing Chemical Equations

Balancing chemical equations involves ensuring that the number of atoms for each element is the same on both sides of the equation. This is crucial for obeying the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. Techniques such as adjusting coefficients and using the smallest whole numbers help achieve balance.
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Balancing Chemical Equations

Molecular vs. Ionic Equations

Molecular equations represent the complete chemical formulas of reactants and products, while ionic equations show the ions present in solution. The net ionic equation is derived from the ionic equation by removing spectator ions—those that do not participate in the reaction—thus highlighting the actual chemical change occurring.
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Molecular and Complete Ionic Equations Example

Net Ionic Equations

A net ionic equation focuses on the species that undergo a change during the reaction, omitting the spectator ions. This equation provides a clearer picture of the actual chemical process, allowing for a better understanding of the reaction dynamics. It is particularly useful in reactions involving soluble ionic compounds in aqueous solutions.
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Net Ionic Equations
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